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2. ATOMIC STRUCTURE
| Term | Definition |
|---|---|
| DALTON: ATOMS | 1. all matter is composed of atoms 2. atoms cannot be created or destroyed 3. atoms of different elements are different 4. atoms can combine to form molecules |
| ATOMIC RADIUS | 10^(-10)m |
| NUCLEAR RADIUS | 10^(-15)m |
| ATOMIC NUMBER | the number of protons in the nucleus |
| MASS NUMBER | the number of protons plus the number of neutrons in an atom |
| ISOTOPES | Atoms of the same element with different mass numbers/different numbers of neutrons |
| ISOTOPES PROPERTIES | 1. same chemical properties 2. different physical properties: melting and boiling points |
| ALPHA PARTICLES | too little neutrons 2 protons + 2 neutrons |
| BETA PARTICLES | too much neutrons electron from neutron decay |
| GAMMA RAYS | electromagnetic radiation |
| CARBON14 DATING | neutron => proton and electron, electron released as beta particle |
| IONS | kation+ anion- |
| MASS SPECTROMETER | vaporization ionization acceleration deflection detection |
| RELATIVE ATOMIC MASS | is the average mass of an atom of an element, taking into account all its isotopes and their relative abundance, compared to one atom of carbon12 |
| ABSORPTION SPECTRUM | when light is passed through something, some colours are missing |
| EMISSION SPECTRUM | when high voltage is applied, then lines are seen |
| ENERGY OF PHOTONS | the energy of a photon is directly proportional to its frequency and inversely proportional to its wavelength |
| FIRST IONIZATION ENERGY | the minimum energy required to remove one mol of electrons from one mole of gaseous atoms in their ground state |
| PATTERNS IN IONIZATION ENERGIES | there is in increase in successive ionization energies there are jumps when electrons are removed from levels closer to the nucleus |
| WAVE AND PARTICLES MODELS | sometimes as wave: electrons through graphite, sometimes as particles |
| UNCERTAINTY PRINCIPLE, HEISENBERG | we cannot know where an electron is at a given moment in time, we only can get the probability picture where it is likely to be |
| ORBITAL | a wave description of an electron, shows the volume of space where the electron is likely to be |
| S ORBITAL | spherical |
| P ORBITAL | 3 p orbitals 2x1, arranged at right angles with the nucleus |
| D ORBITAL | 5 d orbitals 4x1, right angles with nucleus |
| PAULI EXCLUSION PRINCIPLE | no more than two electrons can occupy any one orbital, and if two electrons are in the same orbital they must spin in opposite directions |
| AUFBAU PRINCIPLE | electrons are placed into orbitals of lowest energy first |
| COPPER AND CROMIUM | after e3, e4 and e5 are taken simultaneously |
| IF TWO ELECTRONS IN SAME SUBSHELL | easier to remove one because of repulsive force from other |
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izzy-
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